Which of the following molecules will show a | vedclass

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(C) molecule shows a dipole moment if it has a net non-zero dipole moment due to its geometry and the electronegativity difference between atoms.$CH_4

Vedclass · Accepted Answer

Chloroform

Vedclass · Answer

(C) molecule shows a dipole moment if it has a net non-zero dipole moment due to its geometry and the electronegativity difference between atoms.$CH_4$ (Methane) and $CCl_4$ (Carbon tetrachloride) have a tetrahedral geometry,which results in the cancellation of individual bond dipoles,leading to a net dipole moment of $0$.$CO_2$ (Carbon dioxide) is a linear molecule where the two $C=O$ bond dipoles cancel each other out,resulting in a net dipole moment of $0$.$CHCl_3$ (Chloroform) has a tetrahedral geometry,but because the atoms attached to the central carbon are not identical ($3$ $Cl$ atoms and $1$ $H$ atom),the bond dipoles do not cancel out,resulting in a net dipole moment. Thus,the correct option is $(C)$.

Which of the following molecules will show a dipole moment?

Similar Questions

Molecular $AB$ has a bond length of $1.61\,\mathring{A}$ and a dipole moment of $0.38\,D$. The fractional charge on each atom (absolute magnitude) is $(e_0 = 4.802 \times 10^{-10}\,esu)$

Pick out the molecule which has zero dipole moment.

$(a)$ Discuss the significance/applications of dipole moment.
$(b)$ Represent diagrammatically the bond moments and the resultant dipole moment in $CO_2, NF_3$ and $CHCl_3$.

Which molecule has a zero dipole moment?

Number of compounds from the following with zero dipole moment is . . . . . .
$HF, H_2, H_2S, CO_2, NH_3, BF_3, CH_4, CHCl_3, SiF_4, H_2O, BeF_2$

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